DataResults Table 1 shows the composition of each solution with regards to the

# Dataresults table 1 shows the composition of each

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Data/Results Table 1 shows the composition of each solution with regards to the volume of each component added to the solution. Table 1 Solution #1 Solution #2 Solution #3 Solution #4
Volume, 4 M acetone 10 mL 10 mL 20 mL 10 mL Volume, 1 M HCl 10 mL 10 mL 10 mL 10 mL Volume, 20 mL 10 mL 10 mL 25 mL Volume, 0.00118 M Iodine 10 mL 20 mL 10 mL 5 mL Reaction Time, Trial 1 47 seconds 102 seconds 20 seconds 23 seconds Reaction Time, Trial 2 50 seconds 101 seconds 22 seconds 24 seconds Average Reaction Time 49 seconds 102 seconds 21 seconds 24 seconds Figure 1 shows how the percent difference between the two reaction times were determined for Part 5 of the experiment. Figure 1 Table 2 shows the concentrations of the different solutions (#1-4), along with the initial rate (M/s). Table 2 Solution # [Acetone], M [Iodine], M Initial rate, M/s 1 .20 .20 2 .20 .40
3.92 3 .40 .20 9.52 4 .20 .10 4.17 Figure 2 shows the rate law for the reaction studied in this experiment. Figure 2 Using the rate law, it can be predicted that the theoretical initial rate of the reaction for Solution #4 would be approximately around the same value as Solution #1 and #3, since the manipulation of Iodine has no effect on the rate of the reaction. According to the experimental value, this prediction is correct—the value is very close to that of Solution #1 and #3. It is important to keep the total volume the same throughout the experiment in order to obtain fair and accurate results. If the volume different in each experiment, it would be very difficult to determine which reactant was responsible for the rate change. If more water had been introduced to one

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